Questions: Calculate the amount of heat needed to melt 182 g of solid ethanol (CH3CH2OH) and bring it to a temperature of -16.0°C. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol.

Solution Steps

• Identify the mass of ethanol: \( m = 182 \, \text{g} \).
• Find the heat of fusion for ethanol: \( \Delta H_{\text{fusion}} = 109 \, \text{J/g} \).
• Calculate the heat required to melt the ethanol using the formula: \[ q_{\text{melt}} = m \times \Delta H_{\text{fusion}} \] \[ q_{\text{melt}} = 182 \, \text{g} \times 109 \, \text{J/g} \]

• Since the problem only asks for the heat needed to melt the ethanol and does not involve any temperature change after melting, the total heat required is the same as the heat calculated for melting.
• Perform the multiplication: \[ q_{\text{melt}} = 19838 \, \text{J} \]

• Round the calculated heat to 3 significant digits: \[ q_{\text{melt}} = 1.98 \times 10^4 \, \text{J} \]

Final Answer